How many liters of NH3, at STP, will react with 19.5 g O2 to form NO and H2O? You must show all of your work to receive credit.
4NH3(g) +5O2(g) --> 4NO(g) + 6H2O(g)
How many mols O2 do you have in 19.5 g? That's mols = g/molar mass = ?
The equation tells you that 4 mols NH3 will react with 5 mols O2. So your ? mols O2 will need x mols NH3. x = ?
Now convert x mols NH3 to L NH3 @ STP remembering that 1 mol of a gas will occupy 22.4 L @ STP. Post your work if you get stuck.
To find the number of liters of NH3 that will react with 19.5 g of O2, we need to use stoichiometry. Stoichiometry is the calculation of the quantities of reactants and products in a chemical reaction. In this case, we want to find the number of liters of NH3, so we need to convert mass (g) of O2 to moles, and then use the mole ratio to find the number of moles of NH3.
Here's how to do it step by step:
1. Calculate the number of moles of O2:
To do this, we need to know the molar mass of O2. Oxygen (O) has an atomic mass of 16.00 g/mol, and since O2 is a diatomic molecule, we multiply the atomic mass by 2.
Molar mass of O2 = 16.00 g/mol × 2 = 32.00 g/mol
Now we can calculate the number of moles of O2 by dividing the given mass by its molar mass:
Moles of O2 = mass of O2 / molar mass of O2 = 19.5 g / 32.00 g/mol
2. Use the balanced equation to find the mole ratio between O2 and NH3:
From the balanced equation: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), we can see that the mole ratio between O2 and NH3 is 5:4.
Moles of NH3 = (Moles of O2) × (4 moles of NH3 / 5 moles of O2)
3. Convert moles of NH3 to liters at STP:
At STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 liters.
Liters of NH3 = Moles of NH3 × (22.4 liters / 1 mole)
Now, let's substitute the values into the equations:
Moles of O2 = 19.5 g / 32.00 g/mol
Moles of NH3 = (Moles of O2) × (4 moles of NH3 / 5 moles of O2)
Liters of NH3 = Moles of NH3 × (22.4 liters / 1 mole)
Remember to show all your calculations to receive credit. Let's calculate the answer!